Nanocomposite Perfluorosulfonic Acid/Montmorillonite-Na+ Polymer Membrane as Gel Electrolyte in Hybrid Supercapacitors

Solid-state supercapacitors with gel electrolytes have emerged as a promising field for various energy storage applications, including electronic devices, electric vehicles, and mobile phones. In this study, nanocomposite gel membranes were fabricated using the solution casting method with perfluorosulfonic acid (PFSA) ionomer dispersion, both with and without the incorporation of 10 wt.% montmorillonite (MMT). MMT, a natural clay known for its high surface area and layered structure, is expected to enhance the properties of supercapacitor systems. Manganese oxide, selected for its pseudocapacitive behavior in a neutral electrolyte, was synthesized via direct co-precipitation. The materials underwent structural and morphological characterization. For electrochemical evaluation, a two-electrode Swagelok cell was employed, featuring a carbon xerogel negative electrode, a manganese dioxide positive electrode, and a PFSA polymer membrane serving as both the electrolyte and separator. The membrane was immersed in a 1 M Na2SO4 solution before testing. A comprehensive electrochemical analysis of the hybrid cells was conducted and compared with a symmetric carbon/carbon supercapacitor. Cyclic voltammetric curves were recorded, and galvanostatic charge–discharge tests were conducted at various temperatures (20, 40, 60 °C). The hybrid cell with the PFSA/MMT 10 wt.% exhibited the highest specific capacitance and maintained its hybrid profile after prolonged cycling at elevated temperatures, highlighting the potential of the newly developed membrane.


Introduction
The rising demand for portable and flexible cutting-edge electronics in modern society is significantly boosting the development of cost-effective, lightweight, and sustainable energy storage systems with high power and energy densities.Hybrid supercapacitors have drawn considerable attention in recent years due to their merits of high-power density, superior rate capability, rapid charging/ discharging rate, long cycle life, etc. [1].The development of flexible supercapacitors is a relatively new direction in this field, which is of interest for a number of applications, including electronic devices, electric vehicles, cellular phones, etc. [2][3][4][5][6].
The electrolyte is a key component of the supercapacitor, essential for transferring and balancing charges between the positive and negative electrodes.The interaction between the electrodes and the electrolyte greatly influences the state of the electrode-electrolyte interface and the internal structure of the active materials [7].Therefore, the requirements for the electrolyte are many-it must be stable, have a high ionic conductivity, a wide voltage window, etc. Liquid electrolytes are the most widely used.Solid electrolytes provide a wide window of electrochemical stability and are nonflammable and impermeable, but their low ionic conductivity and poor wetting properties limit their application.Different approaches have been investigated to improve the ionic conductivity, such as the use of a ferroelectric ceramic ion conductor (LiTaO 3 ) to lighten the space charge layer and provide an additional Li + transport pathway [8] or the implementation of lithium superconducting nanowires reinforced with high-performance polymer electrolytes [9].Fast and stable transfer of lithium ions between solid-state electrolytes and electrodes is also a challenge.The formation of an elastic, ultrathin, LiF-rich layer that binds the electrolyte and the lithium anode helps maintain dynamic contact, facilitating ion transfer, promoting uniform lithium deposition, and suppressing side reactions [10].Other alternatives in this direction are polymer electrolytes, which are solid polymer electrolytes and gel electrolytes.
Gel polymer electrolytes (GPEs) bridge liquid and solid polymer electrolytes (SPEs) and serve as both electrolytes and separators [11].They combine the benefits of liquid and solid electrolytes, consisting of a polymer matrix, electrolyte salts, and plasticizers, which enhance ionic conductivity by reducing crystalline content [12].Common GPE materials include polyethylene oxide (PEO), polyvinyl alcohol (PVA), polyacrylonitrile (PAN), and poly(vinylidene fluoride) (PVDF) [13].As these are often derived from nonrenewable sources, researchers are developing alternatives like refractory crosslinking composite GPEs with phosphene and P-N synergistic flame retardants (DPM) to enhance Li + conductivity [14].Additionally, chlorinating electrolytes for sodium-based dual-ion batteries using ethyl methyl carbonate (EMC) improves oxidative stability and compatibility with both cathodes and anodes by forming Cl-containing interface layers [15].GPEs are also used in supercapacitors [16].
Solid polymer electrolytes exhibit excellent processability, are lightweight, and safe to use.In this case, the electrolyte works as a separator for the positive and negative electrodes, and hence, these electrolytes show high ionic conductivity [17].Nafion has been extensively studied for the formation of nano-composite membranes with good performance [18,19].A solid-state symmetric supercapacitor with Nafion electrolytes has been investigated.The relatively high capacitance performances of the device are explained by several factors, including an excellent adhesion realized between electrodes and the Nafion membrane, homogeneous inter-distribution of carbon/Nafion in electrodes, a good contact between electrodes and end-plates, and fast proton transport in smaller carbon pores.The latter phenomenon can be explained by the favorable influence of water molecules around the Nafion binder/electrolyte that are in contact with the carbon pores [20].The combination of Nafion with conducting polymers has been demonstrated to enhance the stability of PAN nanofiber electrodes.This improvement is attributed to Nafion's ability to stabilize the radical cations formed during the charging of the conducting polymer material [21,22].Natural clays, such as montmorillonite (MMT), with multilayer structure and high surface area, are attractive materials for supercapacitors.Natural MMT consists of hydrated sodium-calcium-aluminum-magnesium silicate hydroxides of approximate formula (Na,Ca) 0.33 (Al,Mg) 2 (Si 4 O 10 )(OH) 2 •nH 2 O, where an octahedral layer of AlO 6 units is sandwiched between two tetrahedral layers of SiO 4 units.When the MMT clay is activated with acid, it is used as a solid catalyst for various organic syntheses and is found under the name K10 [23,24].During the acid treatment, the crystal structure of MMT undergoes several changes: the edges of the crystals open and the octahedral cations (Al or Mg) are washed away from the MMT structure, leading to a gradual destruction of the octahedral layers.Thus, the crystal structure of K10 is characterized by partially disrupted octahedral layers located between the tetrahedral silicate layers, resulting in a highly porous substance with an increase in both surface area and pore diameter [25].Furthermore, due to the isomorphous substitution of cations, a constant net negative surface charge is known to develop in K10 [26].A novel hybrid composite based on multi-walled carbon nanotube (MWCNT), acid-leached montmorillonite, and manganese dioxide (MnO 2 ) was prepared using 1.0 M tetraethylammonium tetrafluroborate (Et 4 NBF 4 ) in acetonitrile (AN) as the electrolyte.The asymmetric supercapacitor showed a high energy density of 171 Wh kg −1 at a power density of ~1.98 kW kg −1 .Such high EDLC performance could possibly be linked to the acid-base interaction of montmorillonite through its surface hydroxyl groups with the tetraethylammonium cation [(C 2 H 5 )4N + or TEA + ] of the ionic liquid electrolyte.This study demonstrates the excellent potential of clay-based composites for supercapacitor applications [27].
These studies provoked our interest in preparing a composite membrane based on perfluorosulfonic acid (PFSA) and natural MMT.It is well-known that natural MMT is rich in sodium cations.The sodium cationic charges on the surface and interlayers of clay platelets could lead to the promotion of Na + -conducting pathways.To maximize this effect, a composite PFSA membrane with maximum well-dispersed MMT particles is needed.The addition of MMT particles could effectively improve the stability of the system interface and interfacial stability between polymer electrolytes and electrodes [28].
A study was conducted on PFSA membranes, both with and without montmorillonite (MMT), to assess their effectiveness as separators in an asymmetric supercapacitor.This supercapacitor featured a manganese dioxide (MnO 2 ) positive electrode and a carbon xerogel negative electrode.

Physicochemical Characterization of the MnO 2 and the Polymer Membrane
The X-ray structural characterization of the synthesized MnO 2 is presented in Figure 1.The XRD diffractogram reveals a low degree of crystallinity and the fine-grained nature of the material established by the manifestation of two broad peaks at 2θ 37.5 • and 66.7 • , corresponding to (211) and (112) crystallographic planes of MnO 2 with a structural modification-α (according to ICDD, 2021, No. 00-044-0141 database).These main peaks include other peak positions (at 2θ 36.7 • , 39 • , 65.1 • , 67.6 • , and 68.2 • ) in different directions that did not appear due to the fine dispersion of the α-MnO 2 .In confirmation, the size of the crystallites (t) oriented along the plane (211) is 5 nm, determined by applying Scherer's formula (t = λ/Bcosθ, where λ (in Å) − 1.54056 is X-ray wavelength; θ (in degrees) is the diffraction angle; B (in rad) is line broadening at the full width at half maximum (FWHM).
These studies provoked our interest in preparing a composite me perfluorosulfonic acid (PFSA) and natural MMT.It is well-known tha rich in sodium cations.The sodium cationic charges on the surface and platelets could lead to the promotion of Na + -conducting pathways.To fect, a composite PFSA membrane with maximum well-dispersed needed.The addition of MMT particles could effectively improve the s tem interface and interfacial stability between polymer electrolytes and study was conducted on PFSA membranes, both with and withou (MMT), to assess their effectiveness as separators in an asymmetric su supercapacitor featured a manganese dioxide (MnO2) positive electr xerogel negative electrode.

Physicochemical Characterization of the MnO2 and the Polymer Membran
The X-ray structural characterization of the synthesized MnO2 is p 1. The XRD diffractogram reveals a low degree of crystallinity and the fi of the material established by the manifestation of two broad peaks at 2 corresponding to (211) and (112) crystallographic planes of MnO2 with fication -α (according to ICDD, 2021, № 00-044-0141 database).These m other peak positions (at 2θ 36.7°,39°, 65.1°, 67.6°, and 68.2°) in different not appear due to the fine dispersion of the α-MnO2.In confirmation, th tallites (t) oriented along the plane (211) is 5 nm, determined by apply mula (t = λ/Bcosθ, where λ (in Å) − 1.54056 is X-ray wavelength; θ (in d fraction angle; B (in rad) is line broadening at the full width at half max The transmission electron microscopy (TEM) image (Figure 2) illus of nanosized manganese dioxide particles characterized by varying mor spherical and rod-shaped configurations.These particles exhibit interco The transmission electron microscopy (TEM) image (Figure 2) illustrates the presence of nanosized manganese dioxide particles characterized by varying morphologies such as spherical and rod-shaped configurations.These particles exhibit interconnection, forming a multilayered network structure.The SAED images depict distinct concentric rings, reflecting interplanar spacing within the crystal lattice of α-MnO 2 .
a multilayered network structure.The SAED images depict distinct concentric rings, reflecting interplanar spacing within the crystal lattice of α-MnO2.The specific surface area of the synthesized manganese dioxide is 86 m 2 g −1 .Its average pore diameter is 8.7 nm, a value based on the assumption that the pores have a cylindrical geometry, with p/p0 = 0.99.MnO2 exhibits a narrow pore size distribution in the range between 3 and 18 nm.The аdsorption-desorption isotherm (Figure 3) are II and III types, characteristic of macroporous materials according to the classification of IUPAC [29].The presence of mesopores is also observed.The obtained results show the optimum loading of MMT in the polymer matrix of PFSA is 10 wt.%.PFSA membranes with higher loading led to agglomeration of MMT particles and worsened physicochemical properties.
XRD was employed to identify the intercalated structure of the PFSA/MMT composite membrane.The intercalation of the polymer chains increases the interlayer spacing.It is widely accepted that the driving force for polymer chain intercalation into layered silicate from solution is the entropy gained by the desorption of solvent molecules, which The specific surface area of the synthesized manganese dioxide is 86 m 2 g −1 .Its average pore diameter is 8.7 nm, a value based on the assumption that the pores have a cylindrical geometry, with p/p0 = 0.99.MnO 2 exhibits a narrow pore size distribution in the range between 3 and 18 nm.The adsorption-desorption isotherm (Figure 3) are II and III types, characteristic of macroporous materials according to the classification of IUPAC [29].The presence of mesopores is also observed.The specific surface area of the synthesized manganese dioxide is 86 m 2 g −1 .Its average pore diameter is 8.7 nm, a value based on the assumption that the pores have a cylindrical geometry, with p/p0 = 0.99.MnO2 exhibits a narrow pore size distribution in the range between 3 and 18 nm.The аdsorption-desorption isotherm (Figure 3) are II and III types, characteristic of macroporous materials according to the classification of IUPAC [29].The presence of mesopores is also observed.The obtained results show the optimum loading of MMT in the polymer matrix of PFSA is 10 wt.%.PFSA membranes with higher loading led to agglomeration of MMT particles and worsened physicochemical properties.
XRD was employed to identify the intercalated structure of the PFSA/MMT compo- Polarized optical microscopy (POM) studies clearly indicated a homogeneous nanocomposite membrane, displaying water insolubility and well-dispersed MMT particles.The POM images of PFSA/MMT 10 wt.% are presented in Figure 4.The specific surface area of the synthesized manganese dioxide is 86 m 2 g −1 .Its average pore diameter is 8.7 nm, a value based on the assumption that the pores have a cylindrical geometry, with p/p0 = 0.99.MnO2 exhibits a narrow pore size distribution in the range between 3 and 18 nm.The аdsorption-desorption isotherm (Figure 3) are II and III types, characteristic of macroporous materials according to the classification of IUPAC [29].The presence of mesopores is also observed.The obtained results show the optimum loading of MMT in the polymer matrix of PFSA is 10 wt.%.PFSA membranes with higher loading led to agglomeration of MMT particles and worsened physicochemical properties.
XRD was employed to identify the intercalated structure of the PFSA/MMT composite membrane.The intercalation of the polymer chains increases the interlayer spacing.It is widely accepted that the driving force for polymer chain intercalation into layered silicate from solution is the entropy gained by the desorption of solvent molecules, which The obtained results show the optimum loading of MMT in the polymer matrix of PFSA is 10 wt.%.PFSA membranes with higher loading led to agglomeration of MMT particles and worsened physicochemical properties.
XRD was employed to identify the intercalated structure of the PFSA/MMT composite membrane.The intercalation of the polymer chains increases the interlayer spacing.It is widely accepted that the driving force for polymer chain intercalation into layered silicate from solution is the entropy gained by the desorption of solvent molecules, which offsets the decreased entropy of the confined, intercalated chains [30].Figure 5 shows the diffraction patterns of PFSA, MMT Na + and PFSA/MMT 10 wt.%.
Gels 2024, 10, x FOR PEER REVIEW offsets the decreased entropy of the confined, intercalated chains [30].Figure 5 sh diffraction patterns of PFSA, MMT Na + and PFSA/MMT 10 wt.%.The X-ray diffractogram of the synthesized nanocomposite (PFSA/MMT 10 w veals the structural transformations that occurred within the clay matrix (MMT N intercalation of the polymeric PFSA chains.These are evident through the appea the amorphous halo of the PFSA alongside the peaks of the montmorillonite mat ther evidence of the polymer chains' interposition into the interlayer space of the a shift in the position of its main peak from 7.97° to 6.96° 2θ.This displacement the increase in the interplanar spacing (d001) from 11.08 Å to 12.69 Å, calculated ac to Bragg's law: 2dsinθ = nλ (dhkl-interplanar spacing, hkl-Miller indices; θ-B gle; n-order of the interference, normally n = 1; λ-wavelength).
Figure 6 shows the neat PFSA and composite PFSA/MMT 10 wt.% membra conductivities at different temperatures and 95% RH.Both membranes exhibit a increase in conductivity with increasing temperature.This is because temperatur major role in the kinetics of sodium ion motion in the polymeric membrane, th galleries, and the mobility of polymer chains.The X-ray diffractogram of the synthesized nanocomposite (PFSA/MMT 10 wt.%) reveals the structural transformations that occurred within the clay matrix (MMT Na + ) after intercalation of the polymeric PFSA chains.These are evident through the appearance of the amorphous halo of the PFSA alongside the peaks of the montmorillonite matrix.Further evidence of the polymer chains' interposition into the interlayer space of the MMT is a shift in the position of its main peak from 7.97 • to 6.96 • 2θ.This displacement is due to the increase in the interplanar spacing (d 001 ) from 11.08 Å to 12.69 Å, calculated according to Bragg's law: 2dsinθ = nλ (d hkl -interplanar spacing, hkl-Miller indices; θ-Bragg angle; n-order of the interference, normally n = 1; λ-wavelength).
Figure 6 shows the neat PFSA and composite PFSA/MMT 10 wt.% membrane's ion conductivities at different temperatures and 95% RH.Both membranes exhibit a marked increase in conductivity with increasing temperature.This is because temperature plays a major role in the kinetics of sodium ion motion in the polymeric membrane, the MMT galleries, and the mobility of polymer chains.
offsets the decreased entropy of the confined, intercalated chains [30].Figure 5 sh diffraction patterns of PFSA, MMT Na + and PFSA/MMT 10 wt.%.The X-ray diffractogram of the synthesized nanocomposite (PFSA/MMT 10 w veals the structural transformations that occurred within the clay matrix (MMT N intercalation of the polymeric PFSA chains.These are evident through the appea the amorphous halo of the PFSA alongside the peaks of the montmorillonite mat ther evidence of the polymer chains' interposition into the interlayer space of the a shift in the position of its main peak from 7.97° to 6.96° 2θ.This displacement i the increase in the interplanar spacing (d001) from 11.08 Å to 12.69 Å, calculated ac to Bragg's law: 2dsinθ = nλ (dhkl-interplanar spacing, hkl-Miller indices; θ-Br gle; n-order of the interference, normally n = 1; λ-wavelength).
Figure 6 shows the neat PFSA and composite PFSA/MMT 10 wt.% membra conductivities at different temperatures and 95% RH.Both membranes exhibit a increase in conductivity with increasing temperature.This is because temperature major role in the kinetics of sodium ion motion in the polymeric membrane, th galleries, and the mobility of polymer chains.In comparison to neat PFSA, the conductivity of PFSA/MMT 10 wt.% is highe temperature.At room temperature the ion conductivity of both membranes is sim with the temperature increasing, the difference becomes bigger in favor of the co In comparison to neat PFSA, the conductivity of PFSA/MMT 10 wt.% is higher at any temperature.At room temperature the ion conductivity of both membranes is similar, but with the temperature increasing, the difference becomes bigger in favor of the composite one.The neat PFSA membrane gives an ion conductivity of 23 ms•cm −1 at 60 • C. For the composite membrane, the measured ion conductivity is 29.6 ms•cm −1 at 60 • C, i.e., 29% increase.This clearly indicates that the presence of natural MMT plays a crucial role in improving ion conductivity.This phenomenon could be attributed to the sodium ions found usually in MMT interlayer galleries [31].These galleries served as new ion conduction pathways.

Electrochemical Results
Electrochemical tests, including CV curves and galvanostatic charge/discharge studies at 20 • C, were carried out on the assembled asymmetric supercapacitor cells employing the synthesized membrane with and without MMT.Comparative tests were also conducted on symmetrical supercapacitors equipped with AC carbon electrodes.
The results from galvanostatic charge/discharge (GCD) curves at different current rates are shown in Figure 7.
els 2024, 10, x FOR PEER REVIEW composite membrane, the measured ion conductivity is 29.6 ms.cm −1 at 60 increase.This clearly indicates that the presence of natural MMT plays a c improving ion conductivity.This phenomenon could be attributed to the found usually in MMT interlayer galleries [31].These galleries served as new tion pathways.

Electrochemical Results
Electrochemical tests, including CV curves and galvanostatic charge/di ies at 20 °C, were carried out on the assembled asymmetric supercapacitor ce the synthesized membrane with and without MMT.Comparative tests w ducted on symmetrical supercapacitors equipped with AC carbon electrode The results from galvanostatic charge/discharge (GCD) curves at different are shown in Figure 7.The improvement of the solid-state supercapacitor in an asymmetric (carbon gel in the negative electrode and MnO2 in the positive electrod AX/MnO2) was observed.The mass ratio of the two electrodes was set to 2: which was found to effectively balance the anodic and cathodic overvolta evident that the use of the asymmetric configuration of the solid-state super sents a superior alternative in terms of electrode composition.The combin faradaic and faradaic redox mechanisms in the case of asymmetric configu for synergistic enhancement of performance.It is also evident that the AX metric configuration shows superior performance, with the introduction of membrane structure leading to the highest discharge capacitance.The CV p cell show a typical almost rectangular shape at scan rates from 1 to 40 mV This suggests the excellent capacitive behavior of this cell [33].
The results obtained illustrate the impact of the intercalated stru PFSA/MMT composite membrane.MMT possesses a layered structure, and into the membrane results in an expansion of the distance between the laye The improvement of the solid-state supercapacitor in an asymmetric configuration (carbon gel in the negative electrode and MnO 2 in the positive electrode, denoted as AX/MnO 2 ) was observed.The mass ratio of the two electrodes was set to 2:1 (AX:MnO 2 ), which was found to effectively balance the anodic and cathodic overvoltages [32].It is evident that the use of the asymmetric configuration of the solid-state supercapacitor presents a superior alternative in terms of electrode composition.The combination of non-faradaic and faradaic redox mechanisms in the case of asymmetric configuration allows for synergistic enhancement of performance.It is also evident that the AX/MnO 2 asymmetric configuration shows superior performance, with the introduction of MMT into the membrane structure leading to the highest discharge capacitance.The CV profiles of this cell show a typical almost rectangular shape at scan rates from 1 to 40 mVs −1 (Figure 8).This suggests the excellent capacitive behavior of this cell [33].Cyclic performance emerges as a critical characteristic for assessing SC s charge cycles were executed at a current density of 240 mAg −1 .As depicted the asymmetric cell with a PFSA/MMT electrolyte demonstrates cycling stab 85% retention rate for up to 2000 cycles.This result implies that PAMPS/M stable during charge-discharge cycles and maintains good interfacial contact and activated carbon [34].The voltage profile follows the typical pattern of a tem and also indicates that the developed SC exhibits low resistance.This tributed to the well-homogenized MnO2/AX composite electrode and the fact reactions in the positive electrode proceed faster and are closer to the elect brane.Therefore, diffuse species likely travel shorter distances during the cha charge phases, aided by the presence of MMT.This observation finds support voltammograms in Figure 8 and the GCD curves in Figure 7.The capaci MnO2/AX SC is superior to that of the symmetric SC, although the positive theoretically less electrically conductive than the carbon electrode, a trend similar solid-state SCs [35].The results obtained illustrate the impact of the intercalated structure of the PFSA/MMT composite membrane.MMT possesses a layered structure, and its integration into the membrane results in an expansion of the distance between the layers and favors improving ion transportation.Moreover, this incorporation enhances both the ionic conductivity and tensile strength of PFSA.The PFSA/MMT composite electrolyte exhibits superior integrated characteristics in terms of ionic conductivity and tensile strength when the mass fraction of MMT is approximately 10 wt.% Cyclic performance emerges as a critical characteristic for assessing SC stability.Discharge cycles were executed at a current density of 240 mAg −1 .As depicted in Figure 9, the asymmetric cell with a PFSA/MMT electrolyte demonstrates cycling stability with an 85% retention rate for up to 2000 cycles.This result implies that PAMPS/MMT remains stable during charge-discharge cycles and maintains good interfacial contact with MnO 2 and activated carbon [34].The voltage profile follows the typical pattern of a hybrid system and also indicates that the developed SC exhibits low resistance.This could be attributed to the well-homogenized MnO 2 /AX composite electrode and the fact that surface reactions in the positive electrode proceed faster and are closer to the electrolyte membrane.Therefore, diffuse species likely travel shorter distances during the charge and discharge phases, aided by the presence of MMT.This observation finds support in the cyclic voltammograms in Figure 8 and the GCD curves in Figure 7.The capacitance of the MnO 2 /AX SC is superior to that of the symmetric SC, although the positive electrode is theoretically less electrically conductive than the carbon electrode, a trend observed in similar solid-state SCs [35].
It is clear that temperature has a significant effect on the electrochemical performance of supercapacitors.Higher temperatures generally result in improved electrochemical performance, including increased capacitance and reduced resistance.Additionally, the results in Figure 6 show that, with increasing temperature, the ionic conductivity of the studied membranes also increases significantly, especially on the composite PFSA/MMT 10 wt.%.This prompted us to perform electrochemical studies at higher temperatures to gather information about the stability of the MMT-embedded membrane and its potential suitability for use at elevated temperatures.Electrochemical tests were performed at 40 • C and 60 • C.After the tests at 60 • C, the tests were repeated at room temperature to assess membrane stability.
The results from GCD tests at elevated temperatures are illustrated in Figure 10.
voltammograms in Figure 8 and the GCD curves in Figure 7.The capa MnO2/AX SC is superior to that of the symmetric SC, although the positiv theoretically less electrically conductive than the carbon electrode, a trend similar solid-state SCs [35].It is clear that temperature has a significant effect on the electrochemica of supercapacitors.Higher temperatures generally result in improved el performance, including increased capacitance and reduced resistance.Add results in Figure 6 show that, with increasing temperature, the ionic condu studied membranes also increases significantly, especially on the composit 10 wt.%.This prompted us to perform electrochemical studies at higher tem The discharge capacitance of the supercapacitor decreases as the temperature rises, with a particularly noticeable decrease at 60 °C, accompanied by significant fluctuations.The voltage profiles depict a significant increase in cell resistance, which naturally impacts its performance.It is worth noting that when the supercapacitor was cooled back to 20 °C from 60 °C, the capacitance almost returned to its original value, with very little reduction.This suggests that certain irreversible processes, such as SO4-induced surface redox reactions on the electrodes, occurred during the high-temperature charge-discharge cycles of the supercapacitor [36].Overall, this reduction is insignificant and underscores the durability of the membrane used, confirming its suitability as an electrolyte and separator in supercapacitor systems.This conclusion is further supported by the conducted long-term test after cooling, as depicted in Figure 11.The discharge capacitance of the supercapacitor decreases as the temperature rises, with a particularly noticeable decrease at 60 • C, accompanied by significant fluctuations.The voltage profiles depict a significant increase in cell resistance, which naturally impacts its performance.It is worth noting that when the supercapacitor was cooled back to 20 • C from 60 • C, the capacitance almost returned to its original value, with very little reduction.This suggests that certain irreversible processes, such as SO 4 -induced surface redox reactions on the electrodes, occurred during the high-temperature charge-discharge cycles of the supercapacitor [36].Overall, this reduction is insignificant and underscores the durability of the membrane used, confirming its suitability as an electrolyte and separator in supercapacitor systems.This conclusion is further supported by the conducted long-term test after cooling, as depicted in Figure 11.
bility of the membrane used, confirming its suitability as an electrolyte supercapacitor systems.This conclusion is further supported by the cond test after cooling, as depicted in Figure 11.One potential reason associated with the observed increase in internal resistance, particularly noticeable at 60 • C, is the generation of gases at elevated temperatures due to electrochemical reactions [37].

Conclusions
This study investigated nanocomposite gel membranes fabricated with perfluorosulfonic acid (PFSA) ionomer dispersion, both with and without 10 wt.% natural sodium MMT incorporation.Electrochemical evaluation using a two-electrode cell demonstrated improved performance, notably in the hybrid cell with 10 wt.% MMT, which maintained high specific capacitance even after prolonged cycling at elevated temperatures.These results underscore the significant role of natural sodium MMT in enhancing the ion conductivity of the newly developed membrane, likely attributed to the presence of sodium ions in its enlarged interlayer galleries, highlighting its potential for use in energy storage devices.

Preparation of the MnO 2
Manganese oxide was synthesized by a simple method of chemical precipitation.For the synthesis, KMnO 4 (Valerus Co., Sofia, Bulgaria) was used as a reducing agent and manganese (II) chloride MnCl 2 (Valerus Co., Bulgaria) and distilled water were used as a solvent.The mixing of the two solutions of KMnO 4 and MnCl 2 results in the formation of a fine precipitate.The obtained suspension is stirred for 1 h at room temperature.During synthesis, two phases precipitate, and the supernatant liquid was washed several times with distilled water in a centrifuge (NEYA-16) for 30 min at 5000 rpm.The precipitate obtained was dried at 80 • C in a vacuum dryer.The starting powder material was subjected to an additional heat treatment for 3 h at 200 • C.

Preparation of Composite PFSA/MMT Membranes
A solution casting method was employed to prepare composite membranes using PFSA (FuMA-Tech, Bietigheim-Bissingen, Germany) and MMT (Cloisites Na + , purchased from Southern Clay Products Inc., Louisville, KY, USA), a clay material.The initial solution of PFSA used was 20 wt.% in isopropanol (iPrOH).This solution was diluted to 10 wt.% by adding a solvent while continuously stirring.Subsequently, a specified amount of MMT (10 wt.%) was ultrasonically dispersed into the PFSA solution, followed by mechanical stirring at 60 • C for 2 h to ensure a uniform mixture.The resulting composite mixture was cast onto a glass plate and dried under vacuum at 80 • C for 8 h.After cooling to room temperature, the glass plate was immersed in deionized water to facilitate the peeling of the membrane.Additionally, pure PFSA membranes were fabricated using the same procedure, excluding the addition of clay.The membrane thicknesses were averaged from several measurements taken in different regions of the samples using a Mitutoyo high-accuracy digital micrometer.Before measuring the thickness at room temperature, the membranes were equilibrated in distilled water, and their surfaces were carefully dried with paper.The average membrane thickness is 65 µm ± 2.

Electrode Preparation and Supercapacitor Cell Assembly
The electrodes were prepared in the form of inks and deposited as thin layers by a casting technique.The manganese was used as a positive electrode in the asymmetric cell containing 75 wt.%MnO 2 , 10 wt.% ABG 1005 EG1, 10 wt.% PVDF, 5 wt.% carbon fibers and 1-methyl-2-pyrrolidone solvent.The negative electrode was based on a carbon xerogel (CX) synthesized under laboratory conditions from resorcinol and formaldehyde by microwave synthesis, which has a high surface area (1167 m 2 /g) [38].The electrodes included 80 wt.% activated carbon (AX), 10 wt.% graphite ABG 1005 EG1, 10 wt.% PVDF and 1-methyl-2-pyrrolidone solvent.The electrodes were subjected to drying at 70 • C and subsequent additional heat treatment for 1 h at 120 • C and 20 min at 160 • C in order to improve their mechanical strength.The mass ratio between the positive and negative electrodes is 1:1.Two types of PFSA membranes, with and without MMT-Na + , were used as the electrolyte and separator.Before the electrochemical tests, the membranes were immersed in a 1 M solution of Na 2 SO 4 .For the sake of comparison, symmetrical cells were also assembled with two identical carbon electrodes.

Physicochemical Characterization of Materials
Wide-angle X-ray diffraction (WAXD) scans were obtained using a Bruker D8 Advance ECO diffractometer (Bruker, Billerica, MA, USA), operating at 40 kV and 25 mA in Bragg-Brentano geometry with Ni-filtered Cu Kα radiation and a LynxEye-XE detector over the 2θ range of 5-80 • , with a scanning rate of 0.02 • •s −1 .Its morphology was examined by JEOL JEM 2100, an 80-200 kV (Jeol Ltd., Tokyo, Japan) TEM apparatus.The morphology of PFSA/MMT 10 wt.% was visualized and evaluated with a Leica DMLP Optical Microscope and WAXD.A Fumatech MK3 measurement cell equipped with a potentiostat/galvanostat AutoLab model PGSTAT204FRA32M, Metrohm AG, Herisau, Switzerland, was used to perform impedance measurements.The membrane conductivity was determined by fourprobe impedance measurements in the frequency range of 0.1-10 −6 Hz with a 10 mV signal at 20, 40 and 60 • C and 95% relative humidity.Before each experiment, the cell was left for about 1 h to reach thermal equilibrium.The membrane with ~1.5 cm width was placed on top of the four platinum wire electrodes, which were placed on a Teflon disc with a distance of 1 cm between them.The ionic conductivity was calculated according to equation σ = L/R.A, where σ is the ionic conductivity (in mS•cm −1 ), L is the distance between the electrodes (cm), A is the membrane section area (in cm 2 ) and R is the impedance of the membrane (in ohms).The porous texture of obtained MnO 2 was studied using Quantachrome's AutoSorb iQ apparatus (10215 Timber Ridge Dr, Ashland, VA, USA).The pore size distribution was estimated by using the Barett-Joyner-Halenda method.

Electrochemical Characterization
The electrochemical characteristics of the electrodes were studied in a two-electrode cell (Swagelok-type cell).The capacitor cells were subjected to galvanostatic chargedischarge using an Arbin Instrument System BT-2000 and to long-term cycling with a current of 240 mAg −1 at different temperatures (20, 40, 60 • C).Cyclic voltammetry (CV) measurements were also performed with a Multi PalmSens system (model 4, PalmSens BV, Vleugelboot 22, 3991 CL Houten, The Netherlands).The supercapacitor cells were cycled between 0.05 and 1.6 V at a current load increasing stepwise from 60 to 1200 mAg −1
Gels 2024, 10, x FOR PEER REVIEW 4 of 12 a multilayered network structure.The SAED images depict distinct concentric rings, reflecting interplanar spacing within the crystal lattice of α-MnO2.